CHEM 1110 1st Edition Lecture 9Outline of Last Lecture II. Properties of Aqueous SolutionsIII. Precipitation reactionsIV. Rules for Ionic Compounds in WaterV. Rules for Insoluble Ionic Compounds in WaterOutline of Current Lecture VI. Acids, Bases, and Neutralization ReactionsCurrent LectureI. Acids, Bases, and Neutralization Reactionsa. Acids yield H+ ions in waterb. Bases yield OH- ions in waterc. Strong acids and bases are strong electrolytesd. Weak acids and bases are weak electrolytese. Common strong acids:i. HCl, HClO4, HBr, HNO3, HI, H2SO4f. Common strong bases:i. Group IA metal hydroxides: NaOH, KOH, LiOHii. Heavy 2A metals: NH3, Sr(OH)2, Ca(OH)2, Ba(OH)2iii. Neutralization- reaction of an acid and a baseiv. Salt- ionic compound not containing H+, OH-, or O2-g. Sometimes molecular compounds formed after neutralization reaction is gas withlow solubility in waterh. Sometimes molecular compound formed originally is unstable and breakdown further to yield gaseous producti. Arrhenius theory:i. Acid-yields H+ in waterii. Base- yields OH- in waterj. Bronsted-Lowry theory:i. Acid- proton donorii. Base- proton acceptork. Solution- homogeneous mixture of two or more substancesl. Solute- solution component present in smaller amountm. Solvent- solution component present in larger amountn. Aqueous solution- water as solventThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.o. Concentration- amount of solute dissolved in given quantity of solutionp. Molarity=M=number of moles in one liter solutionq. M=Moles of solute/liters of solutionr. M=Mol/Vs. Chemists often use concentrated stock solutions to prepare dilute